-
acid + metal =
salt + hydrogen
-
acid + metallic oxide =
salt + water
-
acid + carbonate compound =
salt + [acid] water + CO2
-
acid + base =
salt + water
-
hydroxide + nonmetallic oxide =
salt + water
-
metallic oxide + nonmetallic oxide =
salt
-
meatllic oxide + water =
base
-
nonmetallic oxide + water =
acid
-
1. aqueous solutions have a sour taste
2. change color of acid-base indicators
3. some react w/ metals to release H2
4. react w/ oppposite = salt + water
5. conduct an electric current
acids
-
an acid that contains only two different elements: hydrogen and one of the more electronegative elements
binary acid
-
an acid that is a compound of hydrogen, oxygen, and a third element, usually a nonmetal
oxyacid
-
1. aqueous solutions taste bitter
2. change the color of acid-base indicators
3. dilute aqueous solutions feel slippery
4. react w/ opposite = salt + water
5. conduct an electric current
bases
-
a chemical compound that increases the concentration of hydrogen ions (H+) in aqueous solution
Arrhenius acid
-
a substance that increases the concentration of hydroxide ions (OH-) in solution
Arrhenius base
-
an acid that ionizes completely in aqeous solution
strong acid
-
an acid that releases few hydrogen ions in solution
weak acid
-
a molecule or ion that is a proton donor
Bronstead-Lowry acid
-
a moleculeor ion that is a proton acceptor
Bronsted-Lowry base
-
protons are transferred from one reactant (the acid) to another (the base)
Bronsted-Lowry acid-base reaction
-
an acid that can donate only one proton (hydrogen ion) per molecule
monoprotic acid
-
an acid that can donate more than one proton per molecule
polyprotic acid
-
an acid that can donate two protons per molecule
diprotic acid
-
an acid able to donate three protons per molecule
triprotic acid
-
an atom, ion, or molecule that accepts an electro pair to form a covalent bond
Lewis acid
-
an atom, ion, or molecule that donates an electron pair to form a covalent bond
Lewis base
-
the formation of one or more covalent bonds between an electron-pair donor and an electron-pair acceptor
Lewis acid-base reaction
-
the species that remains after a Bronsted-Lowry acid has given up a proton
conjugate base
-
the species that is formed when a Bronsted-Lowry base gains a proton
conjugate acid
-
any species that can act as either an acid or a base
amphoteric
-
the reaction of hydronium ions and hydroxide ions to form water molecules
neutralization
-
an ionic compund composed of a cation from a base and an anion form an acid
salt
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